Chapter 2: Q132CP (page 86)

Ammonium dihydrogen phosphate, formed from the reaction of phosphoric acid with ammonia, is used as a crop fertilizer as well as a component of some fire extinguishers. (a) What are the mass percentages of N and P in the compound? (b) How much ammonia is incorporated into 100. g of compound?

Short Answer

Expert verified

Mass percentage of N is 12.18 % and P=26.94 %.
The mass of ammonia is 14.79 g.

Step by step solution

Finding the mass percentage of N and P

The mass percentage can be calculated as,

$Molecular mss of {NH}_{4} H_{2} {PO}_{4} = 6 \times a . m . of H + a . m . of N + 4 \times a . m . of O + a . m . of P = 6 \times 1 + 14.01 + 4 \times 16 + 30.97 = 114.98 Masspercentage of N = \frac{Atomic mass of N}{Molecular mass {ofNH}_{4} H_{2} {PO}_{4}} \times 100 = \frac{14.01}{114.98} \times 100 Masspercentage (N) = 12.18 % Masspercentage (P) = \frac{Atomic mass of P}{Molecular mass {ofNH}_{4} H_{2} {PO}_{4}} \times 100 = \frac{30.97}{114.98} \times 100 M a s s p e r c e n t a g e (P) = 26.94 %$

Finding the mass of ammonia

The mass percentage can be denoted as,

$Masspercentage ({NH}_{3}) = \frac{Atomic mass of {NH}_{3}}{Molecular mass of {NH}_{4} H_{2} {PO}_{4}} = \frac{17.01}{114.98} \times 100 Masspercentage ({NH}_{3}) = 14.79 % Mass ({NH}_{3}) = Molecular mass of {NH}_{4} H_{2} {PO}_{4} \times Mass percentage ({NH}_{3}) Mass ({NH}_{3}) = 100 g \times 0.1479 = 14.79 g$

Unlock Step-by-Step Solutions & Ace Your Exams!

Full Textbook Solutions
Get detailed explanations and key concepts
Unlimited Al creation
Al flashcards, explanations, exams and more...
Ads-free access
To over 500 millions flashcards
Money-back guarantee
We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Ammonium dihydrogen phosphate, formed from the reaction of phosphoric acid with ammonia, is used as a crop fertilizer as well as a component of some fire extinguishers. (a) What are the mass percentages of N and P in the compound? (b) How much ammonia is incorporated into 100. g of compound?

Short Answer

Step by step solution

Finding the mass percentage of N and P

Finding the mass of ammonia

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Organic Chemistry

Inorganic Chemistry

Making Measurements

Nuclear Chemistry

Ionic and Molecular Compounds

Study anywhere. Anytime. Across all devices.